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Periodic Trends

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kisha
15 diapositives · 294 Views · Sep 27, 2014

This resource explores key concepts of atomic properties and periodic trends, focusing on the effects of protons, electrons, and their positions in the periodic table. Key topics include atomic radius, ionization energy, electron affinity, and ionic radius. It provides sample problems to rank elements by atomic size and ionization energy, highlighting how size increases down a group and decreases across a period. Additionally, it discusses the relationship between atomic structure and properties, offering a visual representation of trends in main group elements.

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Periodic Trends
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  1. Periodic Trends Barbara A. Gage PGCC CHM 1010

  2. Atomic Properties • Depend on: • Number of protons – attractive nuclear force • Number of electrons – shielding effect of electron shells • Distance of electrons from nucleus – distance decreases nuclear force Barbara A. Gage PGCC CHM 1010

  3. Atomic Properties • Atomic radius Metallic and covalent radii. Barbara A. Gage PGCC CHM 1010

  4. Atomic Properties Click on image above to go to the Periodic Trends excelet Barbara A. Gage PGCC CHM 1010

  5. PROBLEM: Using only the periodic table (not Figure 8.15)m rank each set of main group elements in order of decreasing atomic size: SAMPLE PROBLEM 8.3 Ranking Elements by Atomic Size (a) Ca, Mg, Sr (b) K, Ga, Ca (c) Br, Rb, Kr (d) Sr, Ca, Rb PLAN: Elements in the same group increase in size and you go down; elements decrease in size as you go across a period. SOLUTION: (a) Sr > Ca > Mg These elements are in Group 2A(2). (b) K > Ca > Ga These elements are in Period 4. (c) Rb > Br > Kr Rb has a higher energy level and is far to the left. Br is to the left of Kr. (d) Rb > Sr > Ca Ca is one energy level smaller than Rb and Sr. Rb is to the left of Sr. Barbara A. Gage PGCC CHM 1010 Silberberg, Principles of Chemistry

  6. Atomic Properties • Ionization energy energy required to remove an electron from a neutral, gaseous atom Cl (g)  Cl1+ + e- K (g)  K1+ + e- Barbara A. Gage PGCC CHM 1010

  7. First ionization energies of the main-group elements. Figure 8.12 Barbara A. Gage PGCC CHM 1010

  8. PROBLEM: Using the periodic table only, rank the elements in each of the following sets in order of decreasing IE1: SAMPLE PROBLEM 8.4 Ranking Elements by First Ionization Energy (a) Kr, He, Ar (b) Sb, Te, Sn (c) K, Ca, Rb (d) I, Xe, Cs PLAN: IE decreases as you proceed down in a group; IE increases as you go across a period. SOLUTION: (a) He > Ar > Kr Group 8A(18) - IE decreases down a group. (b) Te > Sb > Sn Period 5 elements - IE increases across a period. (c) Ca > K > Rb Ca is to the right of K; Rb is below K. (d) Xe > I > Cs I is to the left of Xe; Cs is furtther to the left and down one period. Barbara A. Gage PGCC CHM 1010 Silberberg, Principles of Chemistry

  9. Table 8.4 Barbara A. Gage PGCC CHM 1010 Silberberg, Principles of Chemistry

  10. Atomic Properties • Electron affinity energy change when an electron is added to a neutral atom to form a negative ion Cl + e-  Cl- K + e-  K1- Barbara A. Gage PGCC CHM 1010

  11. Electron affinities of the main-group elements. Figure 8.14 Barbara A. Gage PGCC CHM 1010 Silberberg, Principles of Chemistry

  12. Figure 8.15 and 8.16 Trends in four atomic properties. Barbara A. Gage PGCC CHM 1010

  13. Ionic Properties • Ionic radius radius of the ionic form of an atom Figure 8.21 Barbara A. Gage PGCC CHM 1010

  14. Ionic vs. atomic radii. Figure 8.22 Barbara A. Gage PGCC CHM 1010 Silberberg, Principles of Chemistry

  15. PROBLEM: Rank each set of ions in order of decreasing size, and explain your ranking: SAMPLE PROBLEM 8.8 Ranking Ions by Size (a) Ca2+, Sr2+, Mg2+ (b) K+, S2-, Cl - (c) Au+, Au3+ PLAN: Compare positions in the periodic table, formation of positive and negative ions and changes in size due to gain or loss of electrons. SOLUTION: (a) Sr2+ > Ca2+ > Mg2+ These are members of the same Group (2A/2) and therefore decrease in size going up the group. The ions are isoelectronic; S2- has the smallest Zeff and therefore is the largest while K+ is a cation with a large Zeff and is the smallest. (b) S2- > Cl - > K+ (c) Au+ > Au3+ The higher the + charge, the smaller the ion. Barbara A. Gage PGCC CHM 1010 Silberberg, Principles of Chemistry